Chemical Kinetics – collision theory

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Presentation transcript:

Chemical Kinetics – collision theory

Main Idea Collision theory relates the rates of chemical reaction to collisions between reacting particles. It is the key to understanding why some reactions are faster than others.

The reaction rate of a chemical reaction is stated as the change in concentration of a reactant or product per unit of time. http://www.wiley.com/college/boyer/0470003790/reviews/kinetics/kinetics_effectors.htm

Reaction rates are determined experimentally.

Collision theory states that atoms, ions, and molecules must collide in order to react. They also must collide with the correct orientation! http://www.wiley.com/college/boyer/0470003790/reviews/kinetics/kinetics_effectors.htm

An activated complex is a temporary, unstable arrangement of atoms in which old bonds are breaking and new bonds are forming. http://www.mts.net/~alou/Chemistry%2012/Unit%203%20-%20Chemical%20Kinetics/Lesson%203%20-%20The%20Collision%20theory.htm

The minimum amount of energy that reacting particles must have to form the activated complex and lead to a reaction is called the activation energy. High activation energy means that few collisions have the required energy and the reaction rate is slow.

http://www.mts.net/~alou/Chemistry%2012/Unit%203%20-%20Chemical%20Kinetics/Lesson%203%20-%20The%20Collision%20theory.htm

http://www.mts.net/~alou/Chemistry%2012/Unit%203%20-%20Chemical%20Kinetics/Lesson%203%20-%20The%20Collision%20theory.htm

http://www.mts.net/~alou/Chemistry%2012/Unit%203%20-%20Chemical%20Kinetics/Lesson%203%20-%20The%20Collision%20theory.htm